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in Chemical Thermodynamics by (80.9k points)
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Assertion: The increase in internal energy (ΔE) for the vaporization of one mole of water at 1 atm and 373 K is zero.

Reason: For all isothermal processes, ΔE = 0

(a) Both A and R are true and R is the correct explanation of A

(b) Both A and R are true but R is not correct explanation of A

(c) A is true but R is false

(d) A and R are false

1 Answer

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Best answer

Correct option  (a) Both A and R are true and R is the correct explanation of A

Explanation:

At 373 K or 100°C, the water starts boiling and at this temperature the vaporization of water is an isothermal process. The internal energy change (ΔE), depends only on temperature and at constant temperature, the internal energy of the gas remains constant, i.e., ΔE is zero.

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